The complete combustion of acetylene, c2h2(g), produces 1300. kj of energy per mole of acetylene consumed. how many grams of acetylene must be burned to produce enough heat to raise the temperature of 1.00 gal of water by 12.0°c if the process is 88.0% efficient? assume the density of water is 1.00 g/cm3.

The combustion of acetylene produces a tremendous amount of energy 3.34g of acetylene is required in the reaction.

Let us calculate the energy absorbed by the water, this will give us the theoretical amount of acetylene.

ΔH = mcθ

m = mass of water

c = heat capacity of water = 4.18 J/g/°C

θ = temperature rise = 12.0°C

Volume of water =  1.00 gal = 3785cm^3

Density of water = 1.00 g/cm3

Mass of water = 3785 g

Substituting values;

ΔH = 3785 g × 4.18 J/g/°C ×  12.0°C

ΔH = 189.86 KJ

If 1 mole of acetylene yield 1300. kJ of energy

x moles yields  189.86 KJ

x =   189.86 KJ ×  1 mole/ 1300. kJ

x =e = 0.146 moles

Mass of acetylene = 0.146 moles × 26 g/mol = 3.796 g

This is the theoretical mass of acetylene required.

Actual mass of acetylene required is obtained from;

88 = actual/3.796 g × 100/1

actual = 88 × 3.796 g/ 100

actual = 3.34g

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you need to take a look at the periodic system in order to sort these elements into pairs that would most likely exhibit similar chemical properties. first, you need to find elements that are found in the same group (groups are vertical in the periodic system), and then to see whether they have the same valence number. if they meet these criteria, they will have similar properties.

the first pair: ne (neon) and kr (krypton), are noble gases found in group 8

the second pair: li (lithium) and k (potassium), found in group 1

the third pair: s (sulfur) and te (tellurium), found in group 6

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